A solution is prepared by dissolving 250g of glucose (C6H1206) in 375g of water. The final volume of the solution is 550 mL. Calculate the concentration in each of the following units. (a) molarity, (b) molality, (c) mass percent, (d) mole fraction.

An aqueous solution is 40.0% by mass silver nitrate, AgNO3, and has a density of 1.47 g/mL. The molality of silver nitrate in the solution is m.

Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO3 (ag), (b. ) 50.0 mg of an aqueous solution that is 1.50 m NaCl, (c) 75.0 g of an aqueous solution that is 1.50% sucrose (C12H22 11) by mass.

What is the molality of a solution consisting of 9.265 mass % of C2H5OH dissolved in water?

A solution is prepared by dissolving 155.0 mL of methanol (CH3OH, density = 0.791 g/mL) in 250 mL of water (density 1.00 g/mL) to give a final solution volume of 350.0 mL. Calculate the (a) molarity of the solution, (b) %wt/wt, (c) %wt/vol, (d) %vol/vol

Calculate the molality of 23.0 g of glucose in 2.40 kg of water.